Use the localized electron model to describe the bonding in \(\mathrm{H}_{2} \mathrm{CO}\) (carbon is the central atom).

To draw the Lewis structure of H2CO, we first need to count the total number of valence electrons for each atom. Hydrogen has 1 valence electron, Carbon has 4 valence electrons, and Oxygen has 6 valence electrons. The molecule's total valence electrons are: 2 (Hydrogen atoms) x 1 (valence electrons each) + 1 (Carbon atom) x 4 (valence electrons) + 1 (Oxygen atom) x 6 (valence electrons) = 12 valence electrons. We will use the total valence electrons to form bonds between the atoms: 1. Place the least electronegative atom, Carbon, in the center. 2. Attach the other atoms around the central atom with single bonds. 3. Distribute the remaining valence electrons as lone pairs to complete the octet rule for all atoms except hydrogen, which only needs 2 electrons. The Lewis structure of H2CO is: O || C H H

To identify the hybridization of the central carbon atom, we will count the number of electron groups (lone pairs and bonding atoms) surrounding it. In the case of H2CO, there are 3 electron groups surrounding the carbon atom: 1. A double bond with oxygen (1 group as each double bond is considered as one electron group) 2. Two single bonds with two hydrogen atoms. Three electron groups lead to sp2 hybridization.

Based on the sp2 hybridization, the molecular geometry of H2CO will be trigonal planar.

Using the localized electron model, we can describe the bonding in H2CO as follows: 1. The central carbon atom forms three sp2 hybrid orbitals, which are used to form sigma bonds with two hydrogen atoms and one oxygen atom. 2. The oxygen atom forms a sigma (single) bond with the carbon atom. Oxygen also has two lone pairs of electrons in its remaining two p orbitals. 3. The double bond between carbon and oxygen consists of one sigma bond (from the overlap of sp2 orbitals) and one pi bond (from the overlap of unhybridized p orbitals in both carbon and oxygen). In summary, H2CO has a trigonal planar molecular geometry with a carbon central atom in an sp2 hybridization state. The carbon atom forms sigma bonds with hydrogen and oxygen atoms, and a pi bond with the oxygen atom.